Ammonia is manufactured by the Haber Process.
N2 (g) + 3H2 (g) ⇌ 2NH3 (g)
Kp=
The pressure used in the Haber Process is 200 atm.
Explain the effect, if any, of increasing the pressure on the equilibrium yield of ammonia.
The equilibrium constants for Kp and Kc are related by the equation
Kp =
where Δn is the number of moles of reactants minus the number of moles of products.
Calculate the value of Kc at 500K when the value of Kp = 3.55 × 10−2 atm−2.
Include the units for Kc.
[Use the value of R = 0.0821 dm3 atm K−1 mol−1]
A mixture of 1.0 mol of nitrogen and 3.0 mol of hydrogen is left to reach equilibrium at 700 K.
Calculate the total pressure, in atmospheres, needed to produce a yield of 0.30 mol of ammonia at 700 K.
Give your answer to an appropriate number of significant figures.
You must show your working.
[Kp = 7.76 × 10−5 atm−2 at 700 K]
The value of the equilibrium constant, Kp, varies with temperature.
The equation relating the values of the equilibrium constant at two temperatures is
In
The equilibrium constant, K1, for the formation of ammonia is 6.76 × 105 atm−2 when the temperature T1 = 298 K.
The enthalpy change ∆H = −92400 J mol−1.
Calculate the value of the equilibrium constant for this reaction at 310 K.
[Use the value of R = 8.31 J mol−1 K−1]
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